Ammonium nitrite undergoes decomposition to produce only gases as shown below.NH₄NO₂(s) $\rarr$ N₂(g) + 2H₂O(g) How many liters of gas will be produced by the decomposition of 32.0 g of NH₄NO₂ at 525^$\circ$C and 1.5 atm A) 45 L B) 55 L C) 65 L D) 75 L E) None of the above

Question

Quizplus · Accepted Answer

The given reaction shows that 1 mole of ammonium nitrite produces 1 mole of nitrogen gas and 2 moles of water vapor. We need to use the ideal gas law to calculate the volume of nitrogen gas produced:

1. Convert the given mass of ammonium nitrite to moles:

n = 32.0 g / 80.06 g/mol = 0.3995 mol

2. Use the ideal gas law to find the volume of nitrogen gas produced:

PV = nRT

V = nRT / P

V = (0.3995 mol) x (0.08206 L·atm/mol·K) x (798.15 K) / (1.5 atm)

V = 65.49 L

Rounding the answer to the nearest whole number gives us 65 L, which is option C).

Ammonium Nitrite Undergoes Decomposition to Produce Only Gases as Shown →\rarr→

Ammonium Nitrite Undergoes Decomposition to Produce Only Gases as Shown $\rarr$